Question

The data below were collected for this reaction: CH3Cl(g) + 3 Cl2(g) → CCl4(g) + 3...

The data below were collected for this reaction:

CH3Cl(g) + 3 Cl2(g) → CCl4(g) + 3 HCl(g)

[CH3Cl] (M) [Cl2] (M) Initial rate (M/s)
0.067 0.083 0.019
0.134 0.083 0.038
0.134 0.166 0.054
0.268 0.332 0.152

(a) Write an expression for the reaction rate law. (b) Calculate the value of the rate constant, k

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For questions 1 through 3, please use the reaction: CH3Cl(g) + 3 Cl2(g) → CCl4(g) +...
For questions 1 through 3, please use the reaction: CH3Cl(g) + 3 Cl2(g) → CCl4(g) + 3 HCl(g) and experimental evidence: [CH3Cl] (M) [Cl2] (M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.014 0.100 0.200 0.224 What is the rate law for this reaction? Rate = k [CH3Cl]2[Cl2] Rate = k [Cl2]2 Rate = k [CH3Cl] Rate = k [CH3Cl][Cl2] Rate = k [Cl2] Flag this Question Question 2 2 pts Solve for the rate of the reaction if...
1. The rate law for the reaction is: Cl2(g) + CHCl3 (g) = HCl (g) +...
1. The rate law for the reaction is: Cl2(g) + CHCl3 (g) = HCl (g) + CCl4 (g) Is Rate = k [Cl2]^1/2 [CHCl3] What are the units for k, assuming time inow seconds and concentration in mol/L 2. What is the unit for the rate of a chemical reaction and the rate constant for a third-order rate law?
If there is initially 2.55 M of Cl2, solve for the amount of Cl2 that is...
If there is initially 2.55 M of Cl2, solve for the amount of Cl2 that is present after 10 seconds. Please use the reaction: CH3Cl(g) + 3 Cl2(g) → CCl4(g) + 3 HCl(g) and experimental evidence: [CH3Cl [Cl2] (M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.014 0.100 0.200 0.224 (Answers Given): 0.596 M    56.4 M 0.0177 M 1.68 M
The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g) <----> C(s) + 2 Cl2...
The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g) <----> C(s) + 2 Cl2 (g) At 300k a 5L flask originally contained 0.0828M of CCl4, 0.0444 M of C and 0.0546M of Cl2. Determine the concentration of Cl2 when equilibrium is reached.
6A) Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.432 moles of CH2Cl2(g), 0.263 moles...
6A) Consider the following reaction: 2CH2Cl2(g) CH4(g) + CCl4(g) If 0.432 moles of CH2Cl2(g), 0.263 moles of CH4, and 0.590 moles of CCl4 are at equilibrium in a 17.7 L container at 576 K, the value of the equilibrium constant, Kc, is 6B)Consider the following reaction: COCl2(g) CO(g) + Cl2(g) If 3.59×10-3 moles of COCl2, 0.265 moles of CO, and 0.211 moles of Cl2 are at equilibrium in a 12.3 L container at 772 K, the value of the equilibrium...
1) Determine the rate law for the following reaction using the data provided: CO(g) + Cl2(g)...
1) Determine the rate law for the following reaction using the data provided: CO(g) + Cl2(g) -----> COCl2(g) [CO]o (M)     [Cl2]o (M)   Initial Rate (M/s) 0.25 0.40   0.985 0.25 0.80   1.97 1.00 0.80   3.94
Consider the reaction SO2Cl2(g) = SO2(g) + Cl2(g). The rate law for this reaction is rate...
Consider the reaction SO2Cl2(g) = SO2(g) + Cl2(g). The rate law for this reaction is rate = k[SO2Cl2] where k=2.90 ´ 10-4 s-1 at a particular temperature. If the initial [SO2Cl2] = 0.0500 M, what is the initial rate? What is the value of the half-life for this initial concentration of SO2Cl2 ? What will be the half-life if the initial [SO2Cl2] = 0.0250 M What will be the half-life if the initial [SO2Cl2] = 0.100 M What will be...
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2...
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2 ? 2Cl (fast, reversible) Cl + CHCl3 ? HCl + CCl3 (slow) Cl + CCl3 ? CCl4 (fast) What rate law does this mechanism predict? (Choose from the list below and enter your answers in alphabetical order, e.g. ABC ). A)k G) [HCl]1/2 M) [Cl]2 B) [HCl] H) [Cl2]1/2 N) [CHCl3]2 C) [Cl2] I) [Cl]1/2 O) [CCl3]2 D) [Cl] J) [CHCl3]1/2 P) [HCl]2 E)...
Carbon tetrachloride can be produced by the following reaction: CS2(g) + 3 Cl2(g) ⇄ S2Cl2(g) +...
Carbon tetrachloride can be produced by the following reaction: CS2(g) + 3 Cl2(g) ⇄ S2Cl2(g) + CCl4(g) In an experiment, 0.120 mol of CS2 and 0.360 mol of Cl2 were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.040 mol CCl4. Calculate the value of K under the experimental conditions. I did it twice and got 1.44676 and 226.056 but both answers were wrong
For the reaction, A(g) + B(g) => 2 C(g), the following data were obtained at constant...
For the reaction, A(g) + B(g) => 2 C(g), the following data were obtained at constant temperature. Experiment Initial [A], mol/L Initial [B], mol/L Initial Rate, M/min 1 0.10 0.10 2 x 10-4 2 0.30 0.30 5.4 x 10-3 3 0.10 0.30 1.8 x 10-3 4 0.20 0.40 6.4 x 10-3 Which of the following is the correct rate law for the reaction? 1. Rate = k[A][B] 2. Rate = k[A]2[B] 3. Rate = k[A]2[B]2 4. Rate = k[A] 5....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT